객관식
For the following aqueous reaction at 298 K: N2(g) + 3 H2(g) ⇌ 2 NH3(g), what is the value of the equilibrium constant K if the equilibrium concentrations are [N2] = 0.20 M, [H2] = 0.30 M, and [NH3] = 0.40 M?
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16. Chemical Equilibrium
Equilibrium Constant K
Multiple Choice
Given the reaction N_2(g) + 3H_2(g) ightarrow 2NH_3(g), and the following equilibrium concentrations obtained from a graph: [N_2] = 0.20 M, [H_2] = 0.60 M, [NH_3] = 1.20 M, estimate the value of the equilibrium constant K_c for this reaction.
A
K_c = 100
B
K_c = 10
C
K_c = 0.1
D
K_c = 1
검증된 단계별 안내1
Write the balanced chemical equation: \(\mathrm{N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)}\).
Recall the expression for the equilibrium constant \(K_c\) in terms of concentrations:
\(K_c = \frac{[\mathrm{NH_3}]^2}{[\mathrm{N_2}][\mathrm{H_2}]^3}\).
Substitute the given equilibrium concentrations into the expression:
\(K_c = \frac{(1.20)^2}{(0.20)(0.60)^3}\).
Calculate the powers and products in the denominator and numerator separately, keeping track of each step carefully.
Divide the numerator by the denominator to find the numerical value of \(K_c\), which estimates the equilibrium constant for the reaction.
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